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20 November, 05:52

A compound containing xenon and fluorine was prepared by shining sunlight on a mixture of xe (0.339 g) and excess f2 gas. if you isolate 0.437 g of the new compound, what is its empirical formula

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  1. 20 November, 08:25
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    Compound contains Xenon and fluorine

    To find the empirical formula we have to find the ratio of Fluorine to Xenon from finding the moles

    Moles Xe = 0.339 g / 131.29 g/mol = 0.00258

    Moles F = 0.437 - 0.339/18.9984 g/mol = 0.098/18.9984 = 0.005159

    By dividing moles of F by moles of Xe, we get

    0.005159/0.00258 = 2

    So, XeF2 is the empirical formula.
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